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Questions and Answers
What is the atomic number of carbon (C) in the isotope $^{14}C$?
What is the atomic number of carbon (C) in the isotope $^{14}C$?
How many neutrons are in the isotope $^{11}C$?
How many neutrons are in the isotope $^{11}C$?
Which of the following correctly describes a cation?
Which of the following correctly describes a cation?
What differentiates isotopes of the same element?
What differentiates isotopes of the same element?
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Which of these is an example of a polyatomic molecule?
Which of these is an example of a polyatomic molecule?
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How many electrons does a neutral sodium atom (Na) contain?
How many electrons does a neutral sodium atom (Na) contain?
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What is the charge of a monatomic ion that has gained two electrons?
What is the charge of a monatomic ion that has gained two electrons?
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Which of the following is a characteristic of a diatomic molecule?
Which of the following is a characteristic of a diatomic molecule?
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What did Dalton's atomic theory propose about elements?
What did Dalton's atomic theory propose about elements?
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What characteristic of noble gases contributes to their high ionization energy?
What characteristic of noble gases contributes to their high ionization energy?
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Which of the following groups of elements has the lowest electronegativity?
Which of the following groups of elements has the lowest electronegativity?
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What is the primary focus of Rutherford's model of the atom?
What is the primary focus of Rutherford's model of the atom?
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What does the term 'ionization energy' refer to?
What does the term 'ionization energy' refer to?
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Which sequence correctly represents the increase in atomic radius among these elements?
Which sequence correctly represents the increase in atomic radius among these elements?
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Which of the following has the highest electron affinity?
Which of the following has the highest electron affinity?
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What was a major contribution of Chadwick's experiment?
What was a major contribution of Chadwick's experiment?
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Which statement correctly describes the trend of ionization energy in the periodic table?
Which statement correctly describes the trend of ionization energy in the periodic table?
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How do compounds differ from their constituent elements according to Dalton?
How do compounds differ from their constituent elements according to Dalton?
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What is the relative mass of a proton compared to an electron?
What is the relative mass of a proton compared to an electron?
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Which characteristic of an atom is identified by its atomic radius?
Which characteristic of an atom is identified by its atomic radius?
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What is a key feature of the structure of an atom according to Thomson's theory?
What is a key feature of the structure of an atom according to Thomson's theory?
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What is the relationship between ionic compounds and empirical formulas?
What is the relationship between ionic compounds and empirical formulas?
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What occurs to the atomic radius when an ion is formed?
What occurs to the atomic radius when an ion is formed?
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Which of the following correctly defines ionization energy?
Which of the following correctly defines ionization energy?
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What happens to electron affinity in relation to atomic radius?
What happens to electron affinity in relation to atomic radius?
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Which statement correctly describes the atomic radius?
Which statement correctly describes the atomic radius?
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What fundamental property changes for elements organized in the periodic system?
What fundamental property changes for elements organized in the periodic system?
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In which way do positive ions compare to their parent atoms concerning atomic radius?
In which way do positive ions compare to their parent atoms concerning atomic radius?
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What is the first ionization energy of an atom represented by the equation A(g) → A+(g) + e–?
What is the first ionization energy of an atom represented by the equation A(g) → A+(g) + e–?
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How does atomic radius affect ionization energy?
How does atomic radius affect ionization energy?
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In which direction does ionization energy trend within a group in the periodic table?
In which direction does ionization energy trend within a group in the periodic table?
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Which type of elements has the highest electron affinity?
Which type of elements has the highest electron affinity?
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What characterizes the trend of electron affinity within a group of the periodic table?
What characterizes the trend of electron affinity within a group of the periodic table?
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What determines the ability of an atom to attract electrons in a bond?
What determines the ability of an atom to attract electrons in a bond?
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Which element has the highest electronegativity?
Which element has the highest electronegativity?
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How does electronegativity trend across a period in the periodic table?
How does electronegativity trend across a period in the periodic table?
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Study Notes
Atomic Structure
- Atomic Number (Z) represents the number of protons in an atom's nucleus.
- Mass Number (A) represents the total number of protons and neutrons in an atom's nucleus.
- Isotopes are atoms of the same element that have the same number of protons but different numbers of neutrons.
Molecules
- A molecule is a group of two or more atoms held together by chemical bonds.
- Diatomic molecules contain two atoms.
- Polyatomic molecules contain more than two atoms.
Ions
- An ion is an atom or group of atoms that has a net positive or negative charge.
- Cations are ions with a positive charge, formed when a neutral atom loses one or more electrons.
- Anions are ions with a negative charge, formed when a neutral atom gains one or more electrons.
- Monatomic ions contain only one atom.
- Polyatomic ions contain more than one atom.
Dalton's Atomic Theory
- Elements are composed of atoms, which are the smallest unit of an element.
- All atoms of a given element are identical.
- Atoms of different elements are different.
- Compounds are formed when atoms of different elements combine in fixed ratios.
- Chemical reactions involve the rearrangement of atoms, not their creation or destruction.
Rutherford's Model of the Atom
- The atom's positive charge is concentrated in the nucleus.
- The nucleus contains protons, which have a positive charge.
- The nucleus is surrounded by electrons, which have a negative charge.
Chadwick's Experiment
- The discovery of the neutron, a neutral particle found in the nucleus.
Molecular and Empirical Formulas
- A molecular formula shows the exact number of atoms of each element in the smallest unit of a substance.
- An empirical formula shows the simplest whole-number ratio of the atoms in a substance.
Ionic Compounds
- Ionic compounds are formed by the electrostatic attraction between cations and anions.
- The formula of an ionic compound represents the simplest ratio of cations and anions that results in a neutral compound.
- The sum of the charges on the cations and anions in each formula unit must equal zero.
Periodic Trends
- Atomic radius is the distance from the nucleus to the outermost electron shell.
- Ionization energy is the energy required to remove one electron from a gaseous atom.
- Electron affinity is the energy change that occurs when an electron is added to a neutral atom in the gaseous state.
- Electronegativity is the relative ability of an atom to attract electrons in a chemical bond.
Jari-jari Atom (Atomic Radius)
- Atomic radius increases as you move down a group because the number of electron shells increases.
- Atomic radius decreases as you move across a period because the nuclear charge increases, pulling the electrons closer to the nucleus.
Energi Ionisasi (Ionization Energy)
- Ionization energy decreases as you move down a group because the outermost electrons are further from the nucleus and easier to remove.
- Ionization energy increases as you move across a period because the nuclear charge increases, making it more difficult to remove electrons.
Afinitas Elektron (Electron Affinity)
- Electron affinity generally increases as you move across a period because the added electron is closer to the nucleus and experiences a stronger attraction.
- Electron affinity generally decreases as you move down a group because the added electron is further from the nucleus and experiences a weaker attraction.
Kelektronegatifan (Electronegativity)
- Electronegativity increases as you move across a period because the nuclear charge increases, attracting electrons more strongly.
- Electronegativity decreases as you move down a group because the outermost electrons are further from the nucleus and experience a weaker attraction.
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Description
Test your knowledge on atomic structure, molecules, and ions with this comprehensive quiz. Explore concepts such as atomic number, mass number, isotopes, and the types of ions. Challenge yourself and deepen your understanding of fundamental chemistry principles.
